Chapter 20

Question 1

The stronger the oxidizing agent

Answer 1

the weaker the reducing agent that is coupled with it

Question 2

Balancing redox reaction: Under acidic condition

Answer 2

1. Break up the equation into half reactions
2. Balance all elements except for O and H
3. Balance O by adding H2O
4. Balance H by adding H+
5. Balance charge by adding electrons
6. equalize the number of electrons on both sides before adding the 2 equations
7. simplify if needed
8. check to make sure everything is balanced including

Question 3

Balancing redox equations: under basic conditions

Answer 3

1. Break up the equation into half reactions
2. Balance all elements except for O and H
3. Balance O by adding H2O
4. Balance H by adding H+
5. Balance charge by adding electrons
6. equalize the number of electrons on both sides before adding the 2 equations
7. simplify if needed
8. add enough OH- to both sides in order to get rid of H+
9. rewrite H+ and OH- as H2O
10. check to make sure everything is balanced including

Question 4

Galvanic/ Valtic cell

Answer 4

refers to an apparatus that makes used of a spontaneous redox reaction to generate electricity

Question 5

Electrolytic cell

Answer 5

refers to an instrument that uses electricity in order to cause a non spontaneous redox reaction to take place

Question 6

Cathode vs. Anode for galvanic cells

Answer 6

cathode - reduction take places (cations move toward) ; positive
anode - oxidation takes place (anion move toward); negative

Question 7

calculating cell potential under standard conditions

Answer 7

E standard of cell = E red + E oxd
E standard of cell = E cathode - E anode

Question 8

Relationship between Gibbs free energy and reaction potential

Answer 8

delta G = -nF E rxn

Question 9

Constant F

Answer 9

96500 C/mol e-

Question 10

Calculating cell potential under nonstandard conditions

Answer 10

E = E (standard) - 0.0592/n log Q

Question 11

relationship between E standard rxn and equilibrium constant K

Answer 11

E standard rxn = 0.0592/n log K

Question 12

The more positive that value of E standard rxn (what’s K)

Answer 12

greater the value of K

Question 13

The more negative that value of E standard rxn (what’s K)

Answer 13

smaller the value of K

Question 14

Cathode vs. Anode for electrolytic cells

Answer 14

anode - postive; oxidation takes place; oxidation agent
cathode - negative; reduction takes place; reduction agent

Question 15

faradays law

Answer 15

the amount of material produced at an electrode is quantitatively related to the total conducted charge

Question 16

A way to get all 4 aspects of Faraday’s law

Answer 16

1. current (A) x time (s)
2. charge (C)
3. moles of e- transferred
4. moles of reactants reacting and moles of products being produced

Question 17

Amps

Answer 17

1C/ 1s